Explain the heat required to melt one mole of the solid

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Reference no: EM13257471

Suppose a single component material X has a critical temperature of 350.0 K and critical pressure of 7.50 atm. The triple point pressure of X is 0.500 atm. The density of the liquid phase of X is 0.850 g/(cm^3), and the density of the solid phase of X is 0.950 g/(cm^3). The molecular weight of X is 65.0 g/mol. The heat required to melt one mole of the solid phase is 20.0 kJ, the heat required to sublime one mole of the solid phase is 40.0 kJ, and the heat required to vaporize one mole of the liquid phase is 30.0 kJ. You may assume that all of these heats associated with phase transitions are independent of temperature.

a) What is the triple point of material X?

b) Consider melting 3.00 moles of material X at 1.00 atm. Assuming that the melting co-existence curve is a straight line, what is X's normal melting temperature?

Reference no: EM13257471

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